Question 1: (a) The density of mercury is 13.595 g cm^-3 . What will be this value in SI units?

(b) Give the SI units and their symbols for the following physical quantities:

(i) Molar mass

(ii) Force

(iii) Pressure

Question 2. Derive the equation PV = 1*mNu^-2/3

Question 3. Briefly explain the Linde's method of liquefaction of gases.

Question 4. What are liquid crystals? Explain the different types of liquid crystals.

Question 5. Explain the following terms:

(i) Lattice

(ii) Basis

(iii) Unit cell

Question 6. Derive temperature-volume relationship for a reversible adiabatic process.

Question 7. Derive the relation between Δ_rU and  Δ_rH

Question 8. Show that for a system (gas) undergoing isothermal reversible expansion and reversible  compression, the total entropy change is zero.

Question 9. State the integrated form of Clausius- Clapeyron equation and explain different terms  appearing in it. What are the application of this equation?

Question 10. What are non-ideal solutions? Give two examples each of different types of such solutions.

Question 11. Explain steam distillation. What kind of impure compounds can be purified by using  this technique?

Question 12. Derive ΔT_b = ΔK_b m.

Question 13. Draw and explain the phase diagram of KI- H₂O system.  

Question 14. The equilibrium constant for the reaction. H₂(g) + S_(s)  <àH₂ S_(g). is 18.5 at 925 K and 9.25 at 1000 K, respectively . Calculate the standard inthalpy of the reaction. Also calculate ΔrG⁰ and ΔrS⁰ at 925K.

Question 15. Calculate the solubility of CaF₂ in water and 0.10 M NaF.

Question 16. State Faraday's laws of electrolysis. What is a faraday?

Question 17. Describe the main features of an amalgam electrode.

Question 18. What are clock reactions? Explain with the help of suitable examples.

Question 19. For the photochemical decomposition of HI, show that the rate the reaction depends on the intensity of the absorbed light.

Question 20. Explain the following terms:

(i) Emulsions

(ii) Physisorption

(iii) Chemisorption.